[Solved] The ionization constant of chloroacetic acid is 1.35×10−3. What will be the pH of 0.1 M acid and its 0.1 M sodium salt solution? - Chemistry Part-I

Name: Video solution 1: [Solved] The ionization constant of chloroacetic acid is 1.35×10−3. What will be the pH of 0.1 M acid and its 0.1 M sodium salt solution? - Chemistry Part-I
Uploaded: 2023-03-08T19:31:39.000Z
Duration: 17 min
Description: Video solution 1: [Solved] The ionization constant of chloroacetic acid is 1.35×10−3. What will be the pH of 0.1 M acid and its 0.1 M sodium salt solution? - Chemistry Part-I

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Chemistry Part-I

Equilibrium

The ionization constant of chloroacetic acid is 1.35 { 10 }^{

Chemistry Part-I

Class 11

NCERT

Chapter 1: Some Basic Concepts of Chemistry

44 questions

Chapter 2: Structure of Atom

85 questions

Chapter 3: Classification of Elements and Periodicity in Properties

50 questions

Chapter 4: Chemical Bonding and Molecular Structure

44 questions

Chapter 5: States of Matter

28 questions

Chapter 6: Thermodynamics and Thermochemistry

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Chapter 7: Equilibrium

101 questions

Predict if the solutions of the following salts are neutral, acidic or basic.

N a Cl, K B r, N a CN, N H_{4} NO_{3}, N a N O_{2}

and

K F

The ionization constant of chloroacetic acid is

1.35 \times 10^{- 3}

. What will be the

p H

of 0.1 M acid and its 0.1 M sodium salt solution?

Ionic product of water at 310 K is

2.7 \times 10^{- 14}

. What is the

p H

of neutral water at this temperature?

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The ionization constant of chloroacetic acid is $1.35 \times 10^{- 3}$ . What will be the $p H$ of 0.1 M acid and its 0.1 M sodium salt solution?

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Updated on: Mar 24, 2023

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Chemistry Part-I (NCERT)

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The ionization constant of chloroacetic acid is

1.35 \times 10^{- 3}

. What will be the

p H

of 0.1 M acid and its 0.1 M sodium salt solution?

8 mins ago

Discuss this question LIVE

8 mins ago

Text solutionVerified

(i) For acid solution,

[H^{+}] = K_{a} C = 0.00135 \times 0.1 = 0.0116 M

p H = - l o g [H^{+}] = - l o g 0.0116 = 1.936

(ii) For 0.1 M sodium salt solution,
The solution contains sodium salt of chloroacetic acid which is weak acid and strong base.

p K_{a} = - l o g K_{a} = l o g (0.00135) = 2.8697

p K_{w} = 14

l o g c = l o g 0.1 = - 1

p H = 0.5 [p K_{w} + p K_{a} + l o g c] = 0.5 [14 + 2.8697 - 1] = 7.935

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Practice more questions from Chemistry Part-I (NCERT)

Predict if the solutions of the following salts are neutral, acidic or basic.

N a Cl, K B r, N a CN, N H_{4} NO_{3}, N a N O_{2}

and

K F

The ionization constant of chloroacetic acid is

1.35 \times 10^{- 3}

. What will be the

p H

of 0.1 M acid and its 0.1 M sodium salt solution?

Ionic product of water at 310 K is

2.7 \times 10^{- 14}

. What is the

p H

of neutral water at this temperature?

View all

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Question Text	The ionization constant of chloroacetic acid is $1.35 \times 10^{- 3}$ . What will be the $p H$ of 0.1 M acid and its 0.1 M sodium salt solution?
Updated On	Mar 24, 2023
Topic	Equilibrium
Subject	Chemistry
Class	Class 11
Answer Type	Text solution:1 Video solution: 2
Upvotes	271
Avg. Video Duration	11 min

The ionization constant of chloroacetic acid is $1.35 \times 10^{- 3}$ . What will be the $p H$ of 0.1 M acid and its 0.1 M sodium salt solution?

Text solutionVerified

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The ionization constant of chloroacetic acid is 1.35×10−3. What will be the pH of 0.1 M acid and its 0.1 M sodium salt solution?

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The ionization constant of chloroacetic acid is $1.35 \times 10^{- 3}$ . What will be the $p H$ of 0.1 M acid and its 0.1 M sodium salt solution?